Step-by-step explanation:
At constant temperature, the change in Gibbs Free Energy is defined like this:
ΔG = ΔH - T * ΔS
Where ΔG is the change in Gibss Free Energy, ΔH is the change in Enthalpy, T is the temperature in K and ΔS is the change in Entropy.
We are given those values.
ΔH = -92.0 kJ ΔS = -0.198 J/K T = 300 K
If we replace them and solve the equation we will get the answer to our problem.
ΔG = ΔH - T * ΔS
ΔG = -92.0 kJ - 300 K * (-0.198 J/K) * 1 kJ/(1000 J)
ΔG = -92.0 kJ + 0.0594 kJ
ΔG = -91.9 kJ
Answer: ΔG = -91.9 kJ